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			{{short description|Inorganic chemical compound}}
	{{chembox		{{chembox
	| verifiedrevid = 396304777		| verifiedrevid = 435505331
	| Name = Cadmium iodide		| Name = Titanium disulfide
	| ImageFile = Cadmium-iodide-3D-balls.png		| ImageFile = Kristallstruktur Cadmiumiodid.png
	| ImageName = Cadmium iodide		| IUPACName = Titanium(IV) sulfide
			| OtherNames = Titanium Sulfide, titanium sulphide, titanium disulfide, titanium disulphide
	| ImageFile1 = Cadmium-iodide-3D-octahedra.png
	| ImageName1 = Cadmium iodide
	| IUPACName = Cadmium(II) iodide
	| OtherNames = Cadmium diiodide
	| Section1 = {{Chembox Identifiers		| Section1 = {{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 23037		| ChemSpiderID =
			| UNII =
	| UNII_Ref = {{fdacite|correct|FDA}}
	| UNII = 2F2UPU4KCW		| CASNo = 12039-13-3
			| EINECS = 232-223-6
	| InChI = 1/Cd.2HI/h;2*1H/q+2;;/p-2
			| PubChem = 61544
	| SMILES = ..
			| InChI = 1S/2S.Ti
	| InChIKey = OKIIEJOIXGHUKX-NUQVWONBAZ
			| SMILES = S==S
	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/Cd.2HI/h;2*1H/q+2;;/p-2
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = OKIIEJOIXGHUKX-UHFFFAOYSA-L
	| CASNo = 7790-80-9
	| CASNo_Ref = {{cascite|correct|CAS}}
	| EINECS = 232-223-6
	}}		}}
	| Section2 = {{Chembox Properties		| Section2 = {{Chembox Properties
	| Formula = CdI<sub>2</sub>		| Formula = TiS<sub>2</sub>
	| MolarMass = 366.22 g/mol		| MolarMass = 111.997 g/mol
	| Appearance = white to pale yellow crystals		| Appearance = yellow powder
	| Density = 5.640 g/cm<sup>3</sup>, solid		| Density = 3.22 g/cm<sup>3</sup>, solid
	| Solubility = 787 g/L (0 °C) <br> 847 g/L (20 °C) <br> 1250 g/L (100 °C)		| Solubility = insoluble
	| SolubleOther = soluble in ], ], ] and ]		| SolubleOther =
	| MeltingPtC = 387		| MeltingPtC =
	| BoilingPtC = 742		| BoilingPtC =
	}}		}}
	| Section3 = {{Chembox Structure		| Section3 = {{Chembox Structure
	| Coordination = octahedral		| Coordination = octahedral
	| CrystalStruct = ], ], ] P{{overline|3}}m1, No. 164		| CrystalStruct = ], ] P{{overline|3}}m1, No. 164
	| Dipole =		| Dipole =
	}}		}}
	| Section7 = {{Chembox Hazards
	| ExternalMSDS =
	| EUClass = Toxic ('''T''')<br/>Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''')
	| EUIndex = 048-007-00-8
	| RPhrases = {{R23/25}}, {{R33}}, {{R68}}, {{R50/53}}
	| SPhrases = {{S2}}, {{S22}}, {{S45}}, {{S60}}, {{S61}}
	}}
	| Section8 = {{Chembox Related
	| OtherAnions = ]<br />]<br />]
	| OtherCations = ]<br />]
	}}
	}}		}}
			'''Titanium disulfide''' is an ] with the formula ]]<sub>2</sub>. A golden yellow solid with high ],<ref name=smartandmoore /> it belongs to a group of compounds called transition metal di], which consist of the ] ]]<sub>2</sub>. TiS<sub>2</sub> has been employed as a ] material in ].
	'''Cadmium iodide''', CdI<sub>2</sub>, is a chemical compound of ] and ]. It is notable for its ], which is typical for compounds of the form MX<sub>2</sub> with strong ] effects.
			==Structure==
			With a ], TiS<sub>2</sub> adopts a ] (hcp) structure, analogous to ] (CdI<sub>2</sub>). In this motif, half of the octahedral holes are filled with a "]", in this case Ti<sup>4+</sup>.<ref name=smartandmoore>{{cite book|title=Solid State Chemistry: An Introduction, Third Edition|year=2005|publisher=Taylor & Francis|location=Boca Raton, FL|author1=Smart, Lesley E.|author2=Moore, Elaine A.}}</ref><ref name=joannasbook/> Each Ti centre is surrounded by six sulfide ligands in an octahedral structure. Each sulfide is connected to three Ti centres, the geometry at S being pyramidal. Several metal di] adopt similar structures, but some, notably MoS<sub>2</sub>, do not.<ref name=joannasbook>{{cite book|title=Shriver and Atkins' Inorganic Chemistry 5th Edition|year=2010|publisher=Oxford University Press|location=Oxford, England|author1=Overton, Peter|author2=Rourke, Tina|author3=Weller, Jonathan|author4=Armstrong, Mark|author5=Atkins, Fraser}}</ref> The layers of TiS<sub>2</sub> consist of covalent Ti-S bonds. The individual layers of TiS<sub>2</sub> are bound together by ], which are relatively weak intermolecular forces. It crystallises in the ] P{{overline|3}}m1.<ref name=xraydiffraction /> The Ti-S bond lengths are 2.423 Å.<ref>{{cite journal | last1 = Chianelli | first1 = R.R. | last2 = Scanlon | first2 = J.C. | last3 = Thompson | first3 = A.H. | year = 1975 | title = Structure refinement of stoichiometric TiS2 | journal = Materials Research Bulletin | volume = 10 | issue = 12 | pages = 1379–1382 | doi=10.1016/0025-5408(75)90100-2}}</ref>
			]
			===Intercalation===
			{{Further|Intercalation (chemistry)}}
			The single most useful and most studied property of TiS<sub>2</sub> is its ability to undergo intercalation upon treatment with electropositive elements. The process is a ], illustrated in the case of lithium:
			:TiS<sub>2</sub> + Li → LiTiS<sub>2</sub>
			LiTiS<sub>2</sub> is generally described as Li<sup>+</sup>. During the intercalation and deintercalation, a range of stoichimetries are produced with the general formul Li<sub>x</sub>TiS<sub>2</sub> (x < 1). During intercalation, the interlayer spacing expands (the lattice "swells") and the electrical conductivity of the material increases. Intercalation is facilitated because of the weakness of the interlayer forces as well as the susceptibility of the Ti(IV) centers toward reduction. Intercalation can be conducted by combining a suspension of the disulfide material and a solution of the alkali metal in anhydrous ammonia. Alternatively solid TiS<sub>2</sub> reacts with the alkali metal upon heating.
			The ] (RBM), which assumes that ] does not change with intercalation, describes changes in the electronic properties upon intercalation.
			Deintercalation is the opposite of intercalation; the cations diffuse out from between the layers. This process is associated with recharging a Li/TiS<sub>2</sub> battery. Intercalation and deintercalation can be monitored by ]. The microstructure of the titanium disulfide greatly affects the intercalation and deintercalation ]s. Titanium disulfide nanotubes have a higher uptake and discharge capacity than the polycrystalline structure.<ref name=mgbatteries>{{cite journal|title=TiS<sub>2</sub> nanotubes as the cathode materials of Mg-ion batteries|journal=]|year=2004|issue=18|pages=2080–2081|doi=10.1039/b403855j|author1=Tao, Zhan-Liang|author2=Xu, Li-Na|author3=Gou, Xing-Long|author4=Chen, Jun|author5=Yuana, Hua-Tang|pmid=15367984}}</ref> The higher surface area of the nanotubes is postulated to provide more binding sites for the anode ions than the polycrystalline structure.<ref name="mgbatteries"/>
			==Material properties==
			Formally containing the d<sup>0</sup> ion Ti<sup>4+</sup> and closed shell dianion S<sup>2−</sup>, TiS<sub>2</sub> is essentially diamagnetic. Its magnetic susceptibility is 9 x 10<sup>−6</sup> emu/mol, the value being sensitive to stoichiometry.<ref name=IS/> Titanium disulfide is a ], meaning there is small overlap of the ] and ].
			===High pressure properties===
			The properties of titanium disulfide powder have been studied by high pressure ] ] (XRD) at room temperature.<ref name=xraydiffraction>{{cite journal|title=A high pressure x-ray diffraction study of titanium disulfide|journal=Journal of Physics: Condensed Matter|year=2009|volume=21|issue=2|doi=10.1088/0953-8984/21/2/025403|author1=Aksoy, Resul|author2=Selvi, Emre|author3=Knudson, Russell|author4=Ma, Yanzhang|page=025403|pmid=21813976|bibcode=2009JPCM...21b5403A|s2cid=22810398 }}</ref> At ambient pressure, TiS<sub>2</sub> behaves as semiconductor while at high pressures of 8 GPa the material behaves as a semimetal.<ref name=xraydiffraction /><ref name=betsyspaper>{{cite journal|title=Electronic Structure of TiS(2) and its electric transport properties under high pressure|journal=J. Appl. Phys.|year=2011|volume=109|issue=5|doi=10.1063/1.3552299|author1=Bao, L.|author2=Yang, J.|author3=Han, Y.H.|author4=Hu, T.J.|author5=Ren, W.B.|author6=Liu, C.L.|author7=Ma, Y.Z.|author8=Gao, C.X.|pages=053717–053717–5|bibcode=2011JAP...109e3717L}}</ref> At 15 GPa, the transport properties change.<ref name=betsyspaper /> There is no significant change in the density of states at the Fermi level up to 20 GPa and phase change does not occur until 20.7 GPa. A change in the structure of TiS<sub>2</sub> was observed at a pressure of 26.3 GPa, although the new structure of the high pressure phase has not been determined.<ref name=xraydiffraction />
			The unit cell of titanium disulfide is 3.407 by 5.695 ]s. The size of the unit cell decreased at 17.8 GPa. The decrease in unit cell size was greater than was observed for MoS<sub>2</sub> and WS<sub>2</sub>, indicating that titanium disulfide is softer and more compressible. The compression behavior of titanium disulfide is ]. The axis parallel to S-Ti-S layers (c-axis) is more compressible than the axis perpendicular to S-Ti-S layers (a-axis) because of weak van der waals forces keeping S and Ti atoms together. At 17.8 GPa, the c-axis is compressed by 9.5% and the a-axis is compressed by 4%. The longitudinal sound velocity is 5284&nbsp;m/s in the plane parallel to S-Ti-S layers. The longitudinal sound velocity perpendicular to the layers is 4383&nbsp;m/s.<ref name=intercalationwithsns>{{cite journal|title=Intercalation: Building a Natural Superlattice for Better Thermoelectric Performance in Layered Chalcogenides|journal=]|year=2011|volume=40|pages=1271–1280|doi=10.1007/s11664-011-1565-5|author1=Wan,CL|author2=Wang,YF|author3=Wang,N|author4=Norimatsu,W|author5=Kusunoki,M|author6=Koumoto,K|issue=5|bibcode=2011JEMat..40.1271W|s2cid=97106786}}</ref>
	==Uses==		==Synthesis==
			Titanium disulfide is prepared by the reaction of the elements around 500&nbsp;°C.<ref name=IS>{{cite book | last1 = McKelvy | first1 = M. J. | last2 = Glaunsinger | first2 = W. S. | title = Inorganic Syntheses | year = 1995 | chapter = Titanium Disulfide | volume = 30 | pages = 28–32 | doi = 10.1002/9780470132616.ch7| isbn = 978-0-471-30508-8 }}</ref>
	Cadmium iodide is used in ], ], ] and the manufacturing of ].<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref>
			:Ti + 2 S → TiS<sub>2</sub>
			It can be more easily synthesized from ], but this product is typically less pure than that obtained from the elements.<ref name=IS/>
	==Preparation==
			:TiCl<sub>4</sub> + 2 H<sub>2</sub>S → TiS<sub>2</sub> + 4 HCl
	Cadmium iodide is prepared by the addition of cadmium metal, or its oxide, hydroxide or carbonate to ].
			This route has been applied to the formation of TiS<sub>2</sub> films by chemical vapor deposition. ]s and organic ]s can be employed in place of hydrogen sulfide.<ref>{{cite journal | last1 = Lewkebandara | first1 = T. Suren | last2 = Winter | first2 = Charles H. | year = 1994 | title = CVD routes to titanium disulfide films | journal = Advanced Materials | volume = 6 | issue = 3| pages = 237–9 | doi = 10.1002/adma.19940060313 | bibcode = 1994AdM.....6..237L }}</ref>
			A variety of other titanium sulfides are known.<ref>{{cite journal |doi=10.1007/BF02881555|title=The S−Ti (Sulfur-Titanium) system|year=1986|last1=Murray|first1=J. L.|journal=Bulletin of Alloy Phase Diagrams|volume=7|issue=2|pages=156–163}}</ref>
	Also, the compound can be made by heating cadmium with iodine.
			===Chemical properties of TiS<sub>2</sub>===
	==Crystal structure==
			Samples of TiS<sub>2</sub> are unstable in air.<ref name=IS/> Upon heating, the solid undergoes oxidation to ]:
	In cadmium iodide the ] ]s form a hexagonal close packed arrangement while the cadmium ]s fill all of the octahedral sites in alternate layers. The resultant structure consists of a layered lattice. This same basic structure is found in many other ]s and ]s. Cadmium iodide is mostly ] but with partial ] character.<ref>{{Greenwood&Earnshaw2nd|pages=1211–1212}}</ref>
			:TiS<sub>2</sub> + O<sub>2 </sub> → TiO<sub>2</sub> + 2 S
			TiS<sub>2</sub> is also sensitive to water:
			:TiS<sub>2</sub> + 2H<sub>2</sub>O → TiO<sub>2</sub> + 2 H<sub>2</sub>S
			Upon heating, TiS<sub>2</sub> releases sulfur, forming the titanium(III) derivative:
	Cadmium iodide's crystal structure is the prototype on which the crystal structures many other compounds can be considered to be based. Compounds with any of the following characteristics tend to adopt the CdI<sub>2</sub> structure:
			:2 TiS<sub>2</sub> → Ti<sub>2</sub>S<sub>3</sub> + S
			===Sol-gel synthesis===
	* ]s of moderately polarising ]; ]s and ]s of strongly polarising cations
			Thin films of TiS<sub>2</sub> have been prepared by the ] process from ] (Ti(OPr<sup>i</sup>)<sub>4</sub>) followed by ].<ref name=thinfilms>{{cite journal|title=Thio sol-gel synthesis of titanium disulfide thin films and powders using titanium alkoxide precursors|journal=Journal of Non-Crystalline Solids|year=2008|volume=354|issue=15–16|pages=1801–1807|doi=10.1016/j.jnoncrysol.2007.09.005|author1=Let, AL|author2=Mainwaring, DE|author3=Rix, C|author4=Murugaraj, P|bibcode=2008JNCS..354.1801L}}</ref> This method affords amorphous material that crystallised at high temperatures to hexagonal TiS<sub>2</sub>, which crystallization orientations in the , , and directions.<ref name=thinfilms /> Because of their high surface area, such films are attractive for battery applications.<ref name=thinfilms />
	* ]s of dications, i.e. compounds with the general formula M(OH)<sub>2</sub>
	* ]s, ]s and ]s (]ides) of tetracations, i.e. compounds with the general formula MX<sub>2</sub>, where X = S, Se, Te
	==Compounds with the CdI<sub>2</sub> crystal structure==		===Unusual morphologoes of TiS<sub>2</sub>===
			More specialized morphologies—]s, ], whiskers, nanodisks, thin films, fullerenes—are prepared by combining the standard reagents, often TiCl<sub>4</sub> in unusual ways. For example, flower-like morphologies were obtain by treating a solution of sulfur in 1-octadecene with titanium tetrachloride.<ref name=flowerstructure>{{cite journal |title=Liquid-Phase Synthesis of Flower-like and Flake-like Titanium Disulfide Nanostructures |journal=] |year=2009 |volume=21 |pages=1725–1730 |doi=10.1021/cm900110h |author1=Prabakar, S. |author2=Bumby, C.W. |author3=Tilley, R.D. |issue=8}}</ref>
	]
	===Iodides===
	], ], ], ], ], ], ], ], ].
	===Chlorides and bromides===		====Fullerene-like materials====
			A form of TiS<sub>2</sub> with a ]-like structure has been prepared using the TiCl<sub>4</sub>/H<sub>2</sub>S method. The resulting spherical structures have diameters between 30 and 80&nbsp;nm.<ref name=fullerenes>{{cite journal |title=Inorganic fullerene-like nanoparticles of TiS<sub>2</sub> |journal=] |year=2005 |volume=411 |issue=1–3 |pages=162–166 |doi=10.1016/j.cplett.2005.05.094 |author1=Margolin, A. |author2=Popovitz-Biro, R. |author3=Albu-Yaron, A. |author4=Rapoport, L. |author5=Tenne, R. |bibcode=2005CPL...411..162M}}</ref> Owing to their spherical shape, these fullerenes exhibit reduced ] and wear, which may prove useful in various applications.
	], ];
			====Nanotubes====
	], ], ], ], ], ].
			Nanotubes of TiS<sub>2</sub> can be synthesized using a variation of the TiCl<sub>4</sub>/H<sub>2</sub>S route. According to ] (TEM), these tubes have an outer diameter of 20&nbsp;nm and an inner diameter of 10&nbsp;nm.<ref name=tinanotubespaper>{{cite journal |title=Low-temperature synthesis of titanium disulfide nanotubes |journal=] |year=2003 |issue=8 |pages=980–981 |doi=10.1039/b300054k |author1=Chen, Jun |author2=Li, Suo-Long |author3=Tao, Zhan-Liang |author4=Gao, Feng |pmid=12744329}}</ref> The average length of the nanotubes was 2-5&nbsp;μm and the nanotubes were proven to be hollow.<ref name="tinanotubespaper"/> TiS<sub>2</sub> nanotubes with open ended tips are reported to store up to 2.5 weight percent hydrogen at 25&nbsp;°C and 4 MPa hydrogen gas pressure.<ref name=hydrogenstorage>{{cite journal |title=Titanium disulfide nanotubes as hydrogen storage materials |journal=] |year=2003 |volume=125 |issue=18 |pages=5284–5285 |doi=10.1021/ja034601c |author1=Chen, J |author2=Li, SL |pmid=12720434 |display-authors=etal}}</ref> Absorption and desorption rates are fast, which is an attractive for hydrogen storage. The hydrogen atoms are postulated to bind to sulfur.<ref name="hydrogenstorage"/>
			====Nanoclusters and nanodisks====
	===Hydroxides of M<sup>2+</sup> ===
			Nanoclusters, or ] of TiS<sub>2</sub> have distinctive electronic and chemical properties due to ] and very large surface to volume ratios. Nanoclusters can be synthesized using ]. The nanoclusters are prepared from a solution of TiCl<sub>4</sub> in tridodecylmethyl ammonium iodide (TDAI), which served as the inverse micelle structure and seeded the growth of nanoclusters in the same general reaction as nanotubes.<ref name="tinanotubespaper"/> Nucleation only occurs inside the micelle cage due to the insolubility of the charged species in the continuous medium, which is generally a low ] inert oil. Like the bulk material, nanocluster-form of TiS<sub>2</sub> is a hexagonal layered structure. . Quantum confinement creates well separated electronic states and increases the ] more than 1 eV in comparison to the bulk material. A spectroscopic comparison shows a large ] for the quantum dots of 0.85 eV.
	], ], ].
			Nanodisks of TiS<sub>2</sub> arise by treating TiCl<sub>4</sub> with sulfur in ].<ref name=nanodisks>{{cite journal |title=Unstable single-layered colloidal TiS<sub>2</sub> nanodisks |journal=] |year=2008 |volume=4 |issue=7 |pages=945–950 |doi=10.1002/smll.200700804 |author1=Park, K.H. |author2=Choi, J. |author3=Kim, H.J. |author4=Oh, D.H. |author5=Ahn, J.R. |author6=Son, S. |pmid=18576280}}</ref>
	===Chalcogenides of M<sup>4+</sup> ===
			==Applications==
	], ], ], ], ];
			:]
			The promise of titanium disulfide as a ] material in ] was described in 1973 by ].<ref>{{cite journal | last1 = Whittingham | first1 = M. Stanley | year = 2004 | title = Lithium Batteries and Cathode Materials | journal = Chem. Rev. | volume = 104 | issue = 10 | pages = 4271–4302 | doi = 10.1021/cr020731c | pmid = 15669156 | s2cid = 888879 }}</ref> The Group IV and V dichalcogenides attracted attention for their high electrical conductivities. The originally described battery used a lithium ] and a titanium disulfide cathode. This battery had high ] and the diffusion of lithium ions into the titanium disulfide cathode was reversible, making the battery rechargeable. Titanium disulfide was chosen because it is the lightest and cheapest chalcogenide. Titanium disulfide also has the fastest rate of lithium ion diffusion into the crystal lattice. The main problem was degradation of the cathode after multiple recycles. This reversible intercalation process allows the battery to be rechargeable. Additionally, titanium disulfide is the lightest and the cheapest of all group IV and V layered dichalcogenides.<ref name=Libatterycathode>{{cite journal|title=High Power Nanocomposite TiS2 Cathodes for All-Solid-State Lithium Batteries|journal=]|year=2011|volume=158|issue=12|pages=A1282–A1289|author1=Trevey, J|author2=Stoldt, C|author3=Lee, S-H|doi=10.1149/2.017112jes|doi-access=free}}</ref> In the 1990s, titanium disulfide was replaced by other cathode materials (manganese and cobalt oxides) in most rechargeable batteries.
			The use of TiS<sub>2</sub> cathodes remains of interest for use in solid-state lithium batteries, e.g., for ] and ]s.<ref name="Libatterycathode"/>
	], ], ], ];
			In contrast to the all-solid state batteries, most lithium batteries employ liquid electrolytes, which pose safety issues due to their flammability. Many different solid electrolytes have been proposed to replace these hazardous liquid electrolytes. For most solid-state batteries, high interfacial resistance lowers the reversibility of the intercalation process, shortening the life cycle. These undesirable interfacial effects are less problematic for TiS<sub>2</sub>. One all-solid-state lithium battery exhibited a power density of 1000 W/kg over 50 cycles with a maximum power density of 1500 W/kg. Additionally, the average capacity of the battery decreased by less than 10% over 50 cycles. Although titanium disulfide has high electrical conductivity, high energy density, and high power, its discharge voltage is relatively low compared to other lithium batteries where the cathodes have higher reduction potentials.<ref name="Libatterycathode"/>
	], ], ], ], ], ].
	===Others===		==Notes==
			{{Reflist|2}}
	], ].
			]
	==References==
	{{reflist}}
			==Further reading==
	{{Cadmium compounds}}
			*http://authors.library.caltech.edu/5456/1/hrst.mit.edu/hrs/materials/public/Titanium_disulfide.htm
			*{{cite journal|title=Surface-assisted synthesis of microscale hexagonal plates and flower-like patterns of single-crystalline titanium disulfide and their field-emission properties|journal=]|year=2008|volume=8|issue=8|pages=2990–2994|doi=10.1021/cg800113n|author1=Tao, Y.|author2=Wu, X.|author3=Zhang, Y.|author4=Dong, L.|author5=Zhu, J.|author6=Hu, Z.}}
			*{{cite journal|title=TiS<sub>2</sub> whisker growth by a simple chemical-vapor deposition method|journal=Journal of Crystal Growth|year=2006|volume=293|issue=1|pages=124–127|doi=10.1016/j.jcrysgro.2006.03.063|author1=Zhang, Y.|author2=Li, Z.|author3=Jia, H.|author4=Luo, X.|author5=Xu, J.|author6=Zhang, X.|author7=Yu, D.J.}}
			{{Titanium compounds}}
	{{DEFAULTSORT:Cadmium Iodide}}
			{{Sulfides}}
	]
	]
	]
	]
	]
			]
	]
			]
	]
			]
	]
	]
	]